3. The two molecules shown below have the same number of carbon atoms. Which do you think will have the larger standard molar entropy? Choose one from the descriptions below. Hint: we did not specifically discuss this in class, but use your knowledge of "disorder" to choose the most sensible answer. You can also do further research on the web. n-hexane iii. iv. V. cyclohexane i. n-hexane, because it has more hydrogen atoms (C6H14) than cyclohexane (C6H12). ii. cyclohexane, because it has fewer hydrogen atoms than n-hexane. They are the same because they have the same number of carbon atoms. n-hexane because it is less rigid than cyclohexane. cyclohexane, because it is more rigid than n-hexane.

3. The two molecules shown below have the same number of carbon atoms. Which do you think will have the larger standard molar entropy? Choose one from the descriptions below. Hint: we did not specifically discuss this in class, but use your knowledge of "disorder" to choose the most sensible answer. You can also do further research on the web. n-hexane iii. iv. V. cyclohexane i. n-hexane, because it has more hydrogen atoms (C6H14) than cyclohexane (C6H12). ii. cyclohexane, because it has fewer hydrogen atoms than n-hexane. They are the same because they have the same number of carbon atoms. n-hexane because it is less rigid than cyclohexane. cyclohexane, because it is more rigid than n-hexane.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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6) Which statement below best describes the Second Law of Thermodynamics? a. A perfectly ordered crystalline solid at zero Kelvin has zero entropy. b. The total entropy is positive for a spontaneous process. c. Energy is conserved. Scanned with CamScanner
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2. Compute for the total entropy change (AS,ntu) of the reaction below in a room temperature of 293 K. 2Na (s) + Cl2 (g) - 2NACI (s) Substance Na (s) Cl2 (g) NaCl (s) S°U/mol.K) 51.30 223.1 72.10 AH (kJ/mol) -411.0
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Do you need to specify the temperature to calculate the entropy change?
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few grams of liquid ammonia (NH3). A few moles of carbon dioxide (CO₂) gas. Change The carbon dioxide expands from a volume of 10.0 L to a volume of 13.0 L while the temperature is held constant at 57.0 °C. The ammonia evaporates at a constant temperature of 11.0 °C. The carbon dioxide is cooled from 87.0 °C to -2.0 °C and is also expanded from a volume of 8.0 L to a volume of 11.0 L. AS AS 0 not enough information AS 0 not enough information AS 0 not enough information
At 0.9 bar of pressure and 373.15 K, the hypothetical transition from liquid to gaseous water will result in what change in the total entropy of the “universe”? No change An increase in the total entropy A decrease in the total entropy Not enough information to determine
Compare the compounds in each set below and decide which is expected to have the higher entropy. Assume all are at the same temperature. a. NH3 (g), ASH3 (g), or PH3 (g) O ASH3 (g) Ο ΝH: (g) O PH3 (g) b. NaCl(s) or NaCl(aq) O NaCl(aq) O NaCI(s) c. C2H4 (g) or N2 (g) (two substances with the same molar mass) ON2 (g) O C,H4 (g) d. C2H; OH(€) or C2H; OH(g) O C, H; OH(g) O C,H,OH(e)
Try Again Your answer is wrong. • Second reaction: Your answer for A Sis incorrect. A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 88.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2Fe₂O3(s) 4Fe(s) + 30₂ (g) ΔΗ = 1648. kJ AS = 4631. AG = J K -24 kJ Which is spontaneous? this…
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of helium (He) gas. A few moles of carbon dioxide (CO₂) gas. A few moles of carbon dioxide (CO₂) gas. Change The helium is compressed from a volume of 11.0 L to a volume of 4.0 L while the temperature is held constant at -6.0 °C. The carbon dioxide is heated from -17.0 °C to 53.0 °C while the volume is held constant at 8.0 L. The carbon dioxide is heated from -8.0 °C to 3.0 °C and also expands from a volume of 10.0 L to a volume of 12.0 L. x AS AS 0 not enough information O AS 0 not enough information O AS 0 not enough information
8. You have discovered a new polymer. A monomer is shown below. To better understand its behavior you calculate its theoretical entropy. With careful measurements you find that it can be in 3 positions around the 1st bond in the chain, 2 around the 2nd bond, 1 around the 3rd bond and 3 around the 4th bond. Further, the ring can be in 4 different positions. What is the entropy in units of KB?